When electricity is passed through a solution of $AlCl_3$,$13.5 \ g$ of $Al$ is deposited. What is the number of Faradays used?

What current strength in $amp$ will be required to liberate $10 \ g$ of chlorine from $NaCl$ solution in one hour?

How many electrons are involved in the reaction when $0.40 \ F$ of electricity is passed through an electrolytic solution?

$A$ current of $2.0 \ A$ is passed for $5 \ hours$ through a molten metal salt,which deposits $22.2 \ g$ of metal (At. wt. $= 177$). The oxidation state of the metal in the metal salt is:

The quantity of electricity required to liberate $5600 \ mL$ of $H_2$ at $STP$ is the same as that required to liberate how many grams of silver (equivalent weight = $108$)?

If in a voltaic cell $5 \ g$ of zinc is consumed,then how many ampere-hours are produced? (Given that the $E.C.E.$ of $Zn$ is $3.387 \times 10^{-7} \ kg/C$)